19868
During electrolysis of \(NaCl\) solution, part of the reaction is \(N{a^ + } + {e^ - } \to Na.\) This is termed as
1 Oxidation
2 Reduction
3 Deposition
4 Cathode reaction
Explanation:
(b)\(\mathop {N{a^ + }}\limits_{ + 1} + {e^ - } \to \mathop {Na}\limits_0 \), means oxidation number is decreased so the reaction is reduction.
ELECTROCHEMISTRY
19869
When a solution of an electrolyte is heated the conductance of the solution
1 Increases because of the electrolyte conducts better
2 Decreases because of the increased heat
3 Decreases because of the dissociation of the electrolyte is suppressed
4 Increases because the electrolyte is dissociated more
Explanation:
(d) Degree of dissociation of weak electrolyte increases on increasing temperature.
ELECTROCHEMISTRY
19870
The passage of current liberates \({H_2}\) at cathode and \(C{l_2}\) at anode. The solution is
1 Copper chloride in water
2 \(NaCl\) in water
3 \({H_2}S{O_4}\)
4 Water
Explanation:
(b) Since discharge potential of water is greater than that of sodium so water is reduced at cathode instead of \(N{a^ + }\) Cathode: \({H_2}O + {e^ - } \to \frac{1}{2}{H_2} + O{H^ - }\) Anode: \(C{l^ - } \to \frac{1}{2}C{l_2} + {e^ - }\).
ELECTROCHEMISTRY
19871
Pure water does not conduct electricity because it
1 Has a low boiling point
2 Is almost totally unionized
3 Is neutral
4 Is readily decomposed
Explanation:
(b)Because it does not have ions.
ELECTROCHEMISTRY
19872
Which is responsible for electrical conduction of molten sodium chloride
19868
During electrolysis of \(NaCl\) solution, part of the reaction is \(N{a^ + } + {e^ - } \to Na.\) This is termed as
1 Oxidation
2 Reduction
3 Deposition
4 Cathode reaction
Explanation:
(b)\(\mathop {N{a^ + }}\limits_{ + 1} + {e^ - } \to \mathop {Na}\limits_0 \), means oxidation number is decreased so the reaction is reduction.
ELECTROCHEMISTRY
19869
When a solution of an electrolyte is heated the conductance of the solution
1 Increases because of the electrolyte conducts better
2 Decreases because of the increased heat
3 Decreases because of the dissociation of the electrolyte is suppressed
4 Increases because the electrolyte is dissociated more
Explanation:
(d) Degree of dissociation of weak electrolyte increases on increasing temperature.
ELECTROCHEMISTRY
19870
The passage of current liberates \({H_2}\) at cathode and \(C{l_2}\) at anode. The solution is
1 Copper chloride in water
2 \(NaCl\) in water
3 \({H_2}S{O_4}\)
4 Water
Explanation:
(b) Since discharge potential of water is greater than that of sodium so water is reduced at cathode instead of \(N{a^ + }\) Cathode: \({H_2}O + {e^ - } \to \frac{1}{2}{H_2} + O{H^ - }\) Anode: \(C{l^ - } \to \frac{1}{2}C{l_2} + {e^ - }\).
ELECTROCHEMISTRY
19871
Pure water does not conduct electricity because it
1 Has a low boiling point
2 Is almost totally unionized
3 Is neutral
4 Is readily decomposed
Explanation:
(b)Because it does not have ions.
ELECTROCHEMISTRY
19872
Which is responsible for electrical conduction of molten sodium chloride
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ELECTROCHEMISTRY
19868
During electrolysis of \(NaCl\) solution, part of the reaction is \(N{a^ + } + {e^ - } \to Na.\) This is termed as
1 Oxidation
2 Reduction
3 Deposition
4 Cathode reaction
Explanation:
(b)\(\mathop {N{a^ + }}\limits_{ + 1} + {e^ - } \to \mathop {Na}\limits_0 \), means oxidation number is decreased so the reaction is reduction.
ELECTROCHEMISTRY
19869
When a solution of an electrolyte is heated the conductance of the solution
1 Increases because of the electrolyte conducts better
2 Decreases because of the increased heat
3 Decreases because of the dissociation of the electrolyte is suppressed
4 Increases because the electrolyte is dissociated more
Explanation:
(d) Degree of dissociation of weak electrolyte increases on increasing temperature.
ELECTROCHEMISTRY
19870
The passage of current liberates \({H_2}\) at cathode and \(C{l_2}\) at anode. The solution is
1 Copper chloride in water
2 \(NaCl\) in water
3 \({H_2}S{O_4}\)
4 Water
Explanation:
(b) Since discharge potential of water is greater than that of sodium so water is reduced at cathode instead of \(N{a^ + }\) Cathode: \({H_2}O + {e^ - } \to \frac{1}{2}{H_2} + O{H^ - }\) Anode: \(C{l^ - } \to \frac{1}{2}C{l_2} + {e^ - }\).
ELECTROCHEMISTRY
19871
Pure water does not conduct electricity because it
1 Has a low boiling point
2 Is almost totally unionized
3 Is neutral
4 Is readily decomposed
Explanation:
(b)Because it does not have ions.
ELECTROCHEMISTRY
19872
Which is responsible for electrical conduction of molten sodium chloride
19868
During electrolysis of \(NaCl\) solution, part of the reaction is \(N{a^ + } + {e^ - } \to Na.\) This is termed as
1 Oxidation
2 Reduction
3 Deposition
4 Cathode reaction
Explanation:
(b)\(\mathop {N{a^ + }}\limits_{ + 1} + {e^ - } \to \mathop {Na}\limits_0 \), means oxidation number is decreased so the reaction is reduction.
ELECTROCHEMISTRY
19869
When a solution of an electrolyte is heated the conductance of the solution
1 Increases because of the electrolyte conducts better
2 Decreases because of the increased heat
3 Decreases because of the dissociation of the electrolyte is suppressed
4 Increases because the electrolyte is dissociated more
Explanation:
(d) Degree of dissociation of weak electrolyte increases on increasing temperature.
ELECTROCHEMISTRY
19870
The passage of current liberates \({H_2}\) at cathode and \(C{l_2}\) at anode. The solution is
1 Copper chloride in water
2 \(NaCl\) in water
3 \({H_2}S{O_4}\)
4 Water
Explanation:
(b) Since discharge potential of water is greater than that of sodium so water is reduced at cathode instead of \(N{a^ + }\) Cathode: \({H_2}O + {e^ - } \to \frac{1}{2}{H_2} + O{H^ - }\) Anode: \(C{l^ - } \to \frac{1}{2}C{l_2} + {e^ - }\).
ELECTROCHEMISTRY
19871
Pure water does not conduct electricity because it
1 Has a low boiling point
2 Is almost totally unionized
3 Is neutral
4 Is readily decomposed
Explanation:
(b)Because it does not have ions.
ELECTROCHEMISTRY
19872
Which is responsible for electrical conduction of molten sodium chloride
19868
During electrolysis of \(NaCl\) solution, part of the reaction is \(N{a^ + } + {e^ - } \to Na.\) This is termed as
1 Oxidation
2 Reduction
3 Deposition
4 Cathode reaction
Explanation:
(b)\(\mathop {N{a^ + }}\limits_{ + 1} + {e^ - } \to \mathop {Na}\limits_0 \), means oxidation number is decreased so the reaction is reduction.
ELECTROCHEMISTRY
19869
When a solution of an electrolyte is heated the conductance of the solution
1 Increases because of the electrolyte conducts better
2 Decreases because of the increased heat
3 Decreases because of the dissociation of the electrolyte is suppressed
4 Increases because the electrolyte is dissociated more
Explanation:
(d) Degree of dissociation of weak electrolyte increases on increasing temperature.
ELECTROCHEMISTRY
19870
The passage of current liberates \({H_2}\) at cathode and \(C{l_2}\) at anode. The solution is
1 Copper chloride in water
2 \(NaCl\) in water
3 \({H_2}S{O_4}\)
4 Water
Explanation:
(b) Since discharge potential of water is greater than that of sodium so water is reduced at cathode instead of \(N{a^ + }\) Cathode: \({H_2}O + {e^ - } \to \frac{1}{2}{H_2} + O{H^ - }\) Anode: \(C{l^ - } \to \frac{1}{2}C{l_2} + {e^ - }\).
ELECTROCHEMISTRY
19871
Pure water does not conduct electricity because it
1 Has a low boiling point
2 Is almost totally unionized
3 Is neutral
4 Is readily decomposed
Explanation:
(b)Because it does not have ions.
ELECTROCHEMISTRY
19872
Which is responsible for electrical conduction of molten sodium chloride